Download 2016

AP Chemistry Summer Assignment
June 2016
RB
Future AP Chemistry Student,
Welcome to AP Chemistry! I am eagerly anticipating a great year of Chemistry. In order to
ensure the best start for everyone next fall, I have prepared a summer assignment that reviews
basic chemistry concepts. There is a multitude of tremendous chemistry resources are available
via the Internet. With the ready access to hundreds of websites either in your home or at the
local library, I am confident that you will have sufficient resources to prepare adequately for the
fall semester. There are few old chemistry textbooks which can be picked up for your reference.
The reference text book as part of AP course is “Chemistry- The central science” by LeMay,
Brown, Burstein.
For those students who have already taken a high school chemistry course, much of the material
in the summer packet will be familiar to you. For those students who will be taking AP
Chemistry as your first high school chemistry course, the problems will help you build a
foundation in chemistry and insure all students are on a relatively even plane. It will be
important for everyone to come to class the first day prepared. While I review, extensive
remediation is not an option as we work towards our goal of being 100% prepared for the AP
Exam in early May 2017. There will be a test covering the basic concepts included in the
summer packet during the first week of school. You can expect a quiz in naming compounds,
identifying ions the first day of school. Based on prior knowledge I can tell you that kids are not
coming prepared with the material even though the assignment is completed. Make sure just
completing assignment should not be the only objective but one should be confident enough to
process the material for application during the school year. The sooner one realizes the easier
the transition to the class.
The course grades are mainly depending on your assessment scores, although lab reports will
also be assigned and evaluated. Do not expect any grade curves or ‘fluff’ assignments in this
class. Assessments are administered and graded as if they are AP exams. Be aggressive in
pursuit of knowledge not just the grades. Prioritize your learning process, do not
procrastinate until the last minute, get help in class, participate in class discussions and seek
support before grades sink below once expectations.
You may contact me by email: ([email protected]) this summer. I will do my best to answer your
questions ASAP.
I hope you are looking forward to an exciting year of chemistry. You are all certainly fine
students, and with plenty of motivation and hard work you should find AP Chemistry a
successful and rewarding experience.
Finally, I recommend that you spread out the summer assignment. Please do not try to
complete it all in the final week of the summer. Chemistry takes time to process and grasp at a
level necessary for success in AP Chemistry. Remember, AP Chemistry is an equivalent course
to Introductory Chemistry in college. Taking a college level course in high school is difficult,
requires dedication, and is a great investment in your education so prepare yourself and arrive
ready to learn.
Have a great summer and enjoy learning chemistry.
Mr. Bulusu
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Utilize Internet Resources to complete the following problems. The URLs below represent a
fraction of the available chemistry addresses available. Please feel free to expand the list and
find other web sites that help prepare you for the coming year. We recommend that you
complete as many online quizzes as possible, take detailed notes, and practice the items
indicated in the packet.
Completed work must be submitted by AUGUST 23rd , Mail the assignments to the school
address or drop them at the main office. Late work will not be accepted. Let me know if
there are any problems in submitting the assignment on time. A list of books prescribed by
the College Board has been provided for your reference. You do not need all the books to
complete the assignment. Any basic chemistry text-book can help you find the information
needed to complete the summer assignment.
http://highschoolhub.org/hub/chemistry.cfm ;
http://www.chemistrycoach.com/home.htm
http://www.collegeboard.com/ap/students/chemistry/index.html
www.chemmybear.com
Balancing equations practice web links
http://science.widener.edu/svb/tutorial/rxnbalancingcsn7.html
http://www.chemistry-drills.com/balance.html
Show work for all the problems. (Hand written or typed solutions will be accepted)
Questions cover topics from general chemistry to basic Mole concepts. Certain topics will be
reviewed during regular school year.
USE SIGNIFICANT DIGITS in problems.
1. Write the most common guidelines to determine significant figures (digits) with an
example?
2. Use factor labeling method to convert the following:
a. 200 meters = ___ miles.
b. 650 in = ____ meters
c. 4 years= _____ seconds.
3. Classify each of the following as units of mass, volume, length, density, energy, or
pressure.
a.Kg
b. Liter
c. m3
d. mm
e. kg/m3
f. Joule
g. atm h. cal.
4. Most laboratory experiments are performed at room temperature at 25˚C. Express this
temperature in:
a.
˚F
B. Kelvin
5. A cylinder rod formed from silicon is 46.0 cm long and has a mass of 3.00 kg. The density
of silicon is 2.33 g/cm3. What is the diameter of the cylinder? (the volume of cylinder is
given by ∏ r2h, where r is the radius and h is the length)
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6. How many significant figures are in each of the following?
a. 1.9200 mm
b. 0.0301001 kJ
c. 6.022 x1023 atoms
g. 460.000 L
e. 0.000036 cm3
f. 10000 g.1001
h. 0.001345
7. Record the following in correct scientific notation:
a. 4050,000,000 cal
b. 0.000123 mol
c. 0.00345 Ǻ
d. 700,000,000 atoms
8. Calculate the following to the correct number of significant figures.
a. 1.270 g / 5.296 cm3
b. 12.235 g / 1.010 L
c. 12 g + 0.38 g
d. 170g + 2.785 g
e. 2.100 x 3.2102
f. 2.35- 0.4 – 1.23 =
9. Give the chemical symbols for the following elements:
a. Carbon
b. sulfur
c. Titanium
d. Nitrogen e. Helium
f. Krypton
g. Fluorine
h. Scandium
I. Arsenic J. Potassium K. Sodium
l. chloride
m. Iron n. Zinc o. tin
10. Write the latin names for each of the elements symbols:
a. Na b. Au
c. Ag
d. Sn
e. Fe
f. Hg
g. K
h. Pb
11. A solid white substance A is heated strongly in the absence of air. It decomposes to form
a new white substance B and a gas C. The gas has exactly the same properties as the
product obtained when carbon is burned in an excess of oxygen. Based on these
observations, can we determine whether solids A and B and the gas C are elements or
compounds? Explain your conclusions for each substance.
12. Label each of the following as either a physical process or a chemical process.
a. Corrosion of aluminum metal.
b. Melting of ice.
c. Pulverizing an aspirin.
d. Digesting a candy bar.
e. Explosion of nitroglycerin.
13. You may notice when water boils, you can see bubbles that rise to the surface of the
water.
a. What is inside these bubbles?
b. Is the boiling of water a chemical or physical change? Explain
14. Dalton assumed that all atoms of the same element were identical in all their
properties. Explain why this assumption is not valid.
Why do we call Ba(NO3)2 barium nitrate, but we call Fe(NO3)2 iron(II) nitrate?
15. Calculate the mass of O2 produced if 3.450 g potassium chlorate is completely
decomposed by heating in presence of a catalyst ( Manganese dioxide).
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16. Write the formula of the following compounds?
a. Calcium sulfate.
b. Ammonium Phosphate
d. potassium perchlorate.
e. Barium Oxide
g. Sodium Perbromate
I. Calcium Iodide
c. Lithium Nitrite
f. Zinc sulfide.
J. Aluminum Carbonate.
17.Define the words: atomic number, atomic mass, mass number, molecular formula,
structural formula, empirical formula, isotopes, cation, anion, metalloid, and allotrope.
18.Determine number of protons and neutrons in each of the following.
a. K1939
b. 2311Na.
c. 20882Pb
d. 3315P
19.White gold is an alloy that typically contains 45.0% by mass gold and the remainder is
platinum. If 154 g of gold are available, how many grams of platinum are required to combine
with the gold to form this alloy?
20.What is the empirical formula of a compound that contains 53.73% Fe and 46.27% of S ?
21.Determine the number of molecules present in 4.50 mol of Nitrogen dioxide, the number
of atoms of oxygen,
22.List the following has diatomic molecule, molecular compound, ionic compound, Atomic
element. Draw particle diagram for each.
a. F2
b. Cl2
c. C d. NaCl e. KF f. CO2
g. H2
h. Ag
i. Rust (Fe2O3)
j. MgO
k. O2
l. I2
m.CO
n. K2CO3
23. State the contribution of the following chemist in one line.
a. Democritus b. Mendeleev c. Henry Becquerel d. Roentgen
f.Faraday
g. Chadwick
h. Millikan
i. Proust
24.What is the difference between a. Oxygen and Oxide
magnesium ion.
e. J.J Thompson
j. Cavendish k. Madam Curie
b. Magensium atom and
25.How many grams of methane (CH4) are present in 10.0 moles of methane gas?
( USE factor labeling method)
26. Calculate the mass in grams of each of the following:
a. 2.01 x 1010 atoms of Mg.
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b. 3.01 x 10 Formula units of BaI2.
27.In an experiment, a student gently heated a hydrated copper compound to remove the water
of hydration. The following data was recorded:
1. Mass of crucible, cover, and contents before heating 23.4 g.
2. mass of empty crucible and cover
18.82 g.
3. mass of crucible, cover, and contents after heating to constant mass 20.94 g.
Calculate the experimental percent of water in the compound.
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28. How do you distinguish: Use a specific example to show the difference?
a. An element from a compound.
b. An element from a mixture.
c. A true solution from a heterogeneous mixture.
d. Distillation from filtration.
e. Chromatography from crystallization
29. An extensive property is one that depends on the amount of the sample. Which of the
following properties are extensive?
a. volume b. density c. temperature d. energy e. melting point. F. pressure
30.A hydrated compound has an analysis of 18.29% Ca, 32.37% Cl, and 49.34% water. What is its
Empirical formula?
31. Name the types of general inorganic reactions with example of each?
32. Define an Arrhenius Acid, Arrhenius base and salt? Give some examples of each.
33. What mass of Iron is required to replace silver from 8.00g of silver nitrate dissolved in
water?
Fe(s) + AgNO3 → Fe(NO3)2 + Ag.
b. Draw a particle diagram to represent the reaction.
34. Write the chemical formulas for the following compounds:
a. Calcium Carbonate b. Ammonium Phosphate c. Sodium Chloride
d. Sodium Oxide e.
Calcium Sulfate
f. Sodium Nitrite g. Magnesium Acetate h. Potassium cyanide
i. Zinc(II) Nitrate j. Iron(III) Phosphate k. Nickel (II) Fluoride
35. Define and give examples a. Law of conservation of mass.
b. Law of multiple proportion.
38.Strontium consists of four isotopes with masses and their percent abundance of 83.9134
amu ( 0.5%), 85.9094 amu (9.9%) , 86.9089 amu (7.0 %) , and 87.9056 amu (82.6 %). Calculate
the atomic mass of Sr ?
39.Nitrogen has two isotopes, N-14 and N-15, with atomic masses of 14.00031 amu and 15.001
amu, respectively. What is the percent abundance of N-15?
40.Write the number of protons and electrons? a P4 molecule b. a PCl5 molecule c. a P3- Ion
d. P 5+ ion.
41.Mercury has an atomic mass of 200.59 amu. Calculate the a.Mass of 3.0 x 1010 atoms.
b.Number of atoms in one nanogram of Mercury.
41.Calculate the molar masses ( g/ mol) of
a. Ammonia ( NH3) b. Baking soda ( NaHCO3))
42.The molecular formula of morphine, a pain-killing narcotic, is C17H19NO3.
a.What is the molar mass?
b.What fraction of atoms in morphine is accounted for by carbon?
c.Which element contributes least to the molar mass?
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43.Complete the list ionic compounds ( name or formula)
a.Cupric Hydroxide
b.Strontium Chromate
c.Ammonium Per chlorate
d.NaHCO3
44.The hormone, thyroxine is secreted by the thyroid gland, and has the formula: C15H17NO4I4.
How many milligrams of Iodine can be extracted from 15.0 Grams of thyroxine?
a. CuSO4
b. Ca(HCO3)2
c. CaSO4. 2 H2O
45. Calculate the percentage by mass of the following compounds:
a. SO3
b. CH3COOCH3
46.Arsenic reacts with chlorine to form a chloride. If 1.587 g of arsenic reacts with 3.755 g of
chlorine, what is the simplest formula of the chloride?
47.Washing soda is a hydrate of sodium carbonate. Its formula is Na2CO3. x H2O. A 2.714 g
Sample of washing soda is heated until a constant mass of 1.006 g of Na2CO3 is reached. What is
x?
48. Explain heat and temperature. Use an example .
49.Determine the empirical and molecular formula of each of the following substances:
a.Ibufuren, a headache remedy contains 75.6 % C, 8.80 % H ,
and 15.5 % O by mass and has a molar mass about 206 g/mol.
50.Write balanced chemical equations for the reactions of sodium with the following nonmetals
to form ionic solids.
a. Nitrogen
b. Oxygen
c. Fluorine
51.Write a balanced equation for the following:
a.Reaction of boron trifluoride gas with water to give liquid hydrogen fluoride and solid boric
acid,(H3BO3).
b.Reaction of magnesium Oxide with Iron to form Iron (III) Oxide and Magnesium.
c.The decomposition of dinitrogen Oxide gas to its elements.
d.The reaction of Calcium Carbide solid with water to form calcium hydroxide and acetylene
(C2H2) gas.
e.The reaction of solid calcium cyan amide (CaCN2) with water to from calcium carbonate and
ammonia gas.
f.Ethane burns in air (Oxygen).
g.Hydrogen reacts with oxygen to from Water.
h.Nitrogen gas reacts with Hydrogen to form Ammonia.
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i.Hydrogen reacts with Iodine gas to form Hydrogen Iodide.
j. Sodium reacts with Iodine gas to form Sodium Iodide.
k.Carbon dioxide combines with water to form carbonic acid.
l.Magnesium and nitrogen gas combine to form magnesium nitride.
m.Conc. Hydrochloric acid reacts with Conc. Sodium hydroxide to form sodium chloride and
water.
52. DEFINE limiting reagent, theoretical yield , and actual yield?
53.Sodium hydroxide reacts with carbondioxide as follows:
2 NaOH(s) + CO2 (g) → Na2CO3 (s) + H2O(l)
Which reagent is the limiting reactant when 1.85 mol of sodium hydroxide and 1.00 mol
carbondixide are allowed to react? How many moles of sodium carbonate can be
produced? How many moles of the excess reactant remain after the completion of the
reaction?
54. WHEN
benzene (C6H6) reacts with bromine (Br2) bromobenzene(C6H5Br) is obtained:
C6H6 + Br2 → C6H5Br + HBr
a.What is the theoretical yield of bromobenzene in this reaction when 30.0g of benzene reacts
with 65.0 g of bromine?
b. If the actual yield of bromobenzene was 56.7 g what was the percentage yield?
55.Define exothermic and endothermic reactions. What happens to the temperature of the
surrounding during endo and exothermic reactions.
56.To prevent a condition called the “bends”, deep sea divers breathe a mixture containing, in
mole percent, 10.0% O2, 10.0% N2 , and 80.0% He.
a.Calculate the molar mass of this mixture.
b.What is the ratio of the density of this gas to that of pure
Oxygen?
57.A 2.0g sample of SX6 (g) has a volume of 329.5 cm3 at 1.00 atm and 20oC. Identify the
element ‘X’. Name the compound.
58.When Hydrogen sulfide gas, H2S, reacts with oxygen, Sulfur dioxide gas and steam are
produced.
a.Write the balanced chemical equation for this reaction.
b.How many liters of sulfur dioxide would be produced from
10.0 l of Oxygen? Assume 100% yield and that all gases are
measured at the same temperature and pressure.
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59.A gaseous mixture contains 5.78 g of methane, 2.15 g of neon, and 6.8 g of sulfur dioxide.
What pressure is exerted by the mixture inside a 75.0 L cylinder at 850C and 751 mm Hg?
60.A sample of Methane gas is at 500C and 20 atm. Would you expect it to behave more ideally
or less ideally if:
a.The pressure was reduced to 1 atm.
b.The temperature were reduced to - 500 C?
61.Define solubility. Prepare a list of solubility rules for ionic compounds in water. ( online
resources) ( IMPORTANT)
62.Define Oxidation and reduction. Provide at least five examples of oxidation and reduction
with chemical reactions. (Example: Rusting of Iron; 4Fe + 3O2 → 2Fe2O3)
63.Define Oxidation number. Find the Oxidation number of
a. Cl in HClO4
b.Sulfur in H2SO4.
c.Phosphorus in PO43d.Manganese in MnO4264.Which of the following statements are always true? Never true? Not always true?
a.A compound wit the molecular formula C6H6 has the same
simplest formula.
b.The mass percent of copper in CuO is less than in Cu2O.
c.The limiting reactant is the one present in the smallest
number of grams.
d.Since C3H6O3 and C6H12O6 reduce to the same formula, they
represent the same compound.
65.A bedroom 11 ft x 12 ft x 8.0 ft contains 35.41 kg of air at 25˚C. Express the volume of the
room in liters, the amount of air in moles (molar mass of air is 29.0 g/mol) and the temperature
in Kelvin.
66.A sample of carbon dioxide gas, CO2 (g), occupies a volume of 5.75 L at 0.890 atm. If the
temperature and the number of moles remain constant, calculate the volume when the
pressure
a.increased to 1.25 atm
b.decrease to 0.350 atm
67.An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmHg and room
temperature is 68˚F. How many moles are present in the flask when the pressure is 1.10 atm
and the temperature is 33˚C?
68.A drum use to transport crude oil has a volume of 162 L. How many water molecules, as
steam, are required to fill the drum at 1.00 atm and 100˚C? What volume of liquid water
(density of water is 1.0 g/cm3) is required to produce that amount of steam?
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69. Define strong electrolyte, weak electrolyte, precipitation reactions and solubility?
70. What is an Activity series of metal? How does it help us in studying properties of elements?
71. Define the terms: Exothermic, endothermic reactions?
How much heat is required to
raise the temperature of 100 grams of water from 250C to 820C?
72. A piece of unknown metal with mass 30 g is heated to 1100C and dropped into 100.0 g of
water at 200C. The final temperature of the system is 25 degree Celsius. What is the specific heat
of the metal?
73.What is a solute and solvent? Define Molarity, Molality, mole-fraction and Mass percent of a
solution?
74.Calculate the molarity of a solution that contains 0.2 mol NH4Br in exactly 200 ml of solution?
75.Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200ml?
76.How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride?
77.The compound adrenaline contains 56.7 % C, 6.56 % H, 28.37% O and 8.28 % N by mass.
What is the empirical formula for adrenaline?
78.DDT, an insecticide harmful to fish, birds, and humans, is produced by the following
reaction:
2C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O
Chloro benzene Choral
DDT
If 1142 g of chlorobenzene is reacted with 485 g of chloral.
a.
b.
c.
d.
What mass of DDT is formed?
Which reactant is limiting? Which is in excess?
What mass of excess reactant is left over?
If the actual yield of DDT is 200.0 g, what is the percent yield?
79.A 2.25 g sample of scandium metal is reacted with excess hydrochloric acid to produce
0.1502 g hydrogen gas. What is the formula of the scandium chloride produced in the
reaction?
80.Differentiate between what happens when the following are dissolved in water. Use a
particular example
A.Polar solute Vs non polar solute.
B. Ionic Vs Molecular
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( Section is followed by naming ions)
AP CHEMISTRY (Common mono, di & polyatomic ions.)
Name ( Ion)
Symbol( Ion)
a) Sodium
b) Potassium
c) Cesium
d) Beryllium
e) Calcium
f) Strontium
g) Barium
h) Gallium
i) Aluminum
j) Nitrogen
k) Arsenic
l) Bismuth
m) Oxygen
n) Fluorine
o) Chlorine
p) Bromine
q) Iodine
Common ions of transition elements
Ion Name
Ion
a) Chromium(III)
b) Manganese(II)
c) Iron(II) or Ferrous
d) Iron(III) or Ferric
e) Cobalt(II)
f) Nickel(II) or nickel
g) Copper(II) or Cupric
h) Zinc
i) Silver
j) Cadmium
k) Mercury(II) or mercuric
I)
Name
a) Acetate
c) Carbonate
e) Chlorite
g) Cyanide
i) Dihydrogen Phosphate
k) Hydrogen Carbonate
m) Hydrogen Sulfite
o) Hydroxide
q) Nitrite
s) Perchlorate
u) Perioxide
Common Polyatomic Ions
Formula
Name
b) Ammonium
d) Chlorate
f) Chromate
h) Dichromate
j) Dihydrogen Phosphate
l) Hydrogen Sulfate
n) Hypochlorite
p) Nitrate
r) Oxalate
t) Permanganate
v) Phosphate
Formula
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w) Sulfate
y) Thiosulfate
Common Acids
Hydrochloric Acid
acid
Carbonic acid
Nitrous acid
Nitric Acid
Chlorous Acid
x) Sulfite
Formula
Common Acids
Phosphoric acid
Formula
Perchloric
Sulfurous Acid
Sulfuric Acid
Hypochlorous Acid
Chloric Acid
Certain prescribed textbooks for AP CHEM. We follow the highlighted book in school for AP
Course.
Bell, Jerry. Chemistry. Bedford, NJ: W. H. Freeman.
Brady, James E., and Fred Senese. Chemistry: Matter and Its Changes. New York: John Wiley &
Sons.
Brown, Theodore E., H. Eugene LeMay, and Bruce E. Bursten. Chemistry: The Central Science.
Upper Saddle River, NJ: Prentice Hall.
Chang, Raymond, and Brandon Cruickshank. Chemistry. New York: McGraw-Hill.
Hill John W., Ralph H. Petrucci, Terry W. McCreary, and Scott S. Perry. General Chemistry: An
Integrated Approach. Upper Saddle River, NJ: Pearson/Prentice Hall.
Kotz, John C., Paul M. Treichel, Gabriela C. Weaver. Chemistry & Chemical Reactivity. Pacific
Grove, CA: Brooks/Cole Thomson Learning.
Masterton, William L., and Cecile N. Hurley. Chemistry: Principles and Reactions. Pacific Grove,
CA: Brooks/Cole Thomson Learning.
Moore, John W., Conrad L. Stanitski, and Peter C. Jurs. Chemistry: The Molecular Science.
Pacific Grove, CA: Brooks/Cole Thomson Learning.
Olmsted, John A., and Gregory M. Williams. Chemistry. New York: John Wiley & Sons.
Silberberg, Martin. The Molecular Nature of Matter and Change. New York: McGraw-Hill.
Spencer, James N., George M. Bodner, and Lyman H. Rickard. Chemistry: Structure and
Dynamics. New York: John Wiley & Sons.
Zumdahl, Steven, and Susan Zumdahl. Chemistry. Boston: Houghton Mifflin
Visit www.collegeboard.com for more information. These books are listed on College Board
website.
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